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THERMOOOOOO Flashcards

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Physics 101 flashcards AP® Physics flashcards
1
Q

system

A

A quantity of matter or a region in
space chosen for study.

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2
Q

surroundings

A

The mass or region outside the
system (we do our measuring in the
surroundings)

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3
Q

Boundary

A

The real or imaginary surface that
separates the system from its
surroundings.
The boundary of a system can be
fixed or movable.

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4
Q

Closed system

A

Closed system (Control mass): matter can not go in
and out of the system
A fixed amount of mass, and no mass can cross its boundary.
But volume can be changed.

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5
Q

Open system

A

Open system (control volume): matter can go in and out the
system
Both mass and energy can cross the boundary of a control volume.
such as a compressor, turbine, or nozzle.

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6
Q

Isolated system

A

➢ An isolated system is a general system where
no mass, heat or work may cross the boundaries.
➢ An isolated system is a closed system with no energy crossing
the boundaries.

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7
Q

Property

A

Any observable macroscopic characteristic of a
system.

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8
Q

Intensive properties:

A

Independent of the mass of a system, such as
temperature, pressure, and density.

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9
Q

Extensive property

A

Those whose values depend on the size—or
extent—of the system: total mass, total volume

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10
Q

Specific property

A

Extensive properties per unit mass

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11
Q

State

A

: condition of system defined by properties

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12
Q

State postulate

A
  • The state of a simple
    compressible system is
    completely specified by two
    independent, intensive
    properties.
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13
Q

Simple compressible system

A

If a system involves no electrical, magnetic, gravitational, motion, and surface tension effects.

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14
Q

Equilibrium (mech, phase, thermal)

A

In an equilibrium state there are no unbalanced potentials (or driving forces) within the
system.

Mech no pressure change
, phase no phase change, thermal all same temp throughout

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15
Q

Process path cycle

A

Process:
Change from State 1 to state 2
Path:
The series of states through which a system passes during a
process.
31
Cycle:
A process during which the initial
and final states are identical.

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16
Q

Iso

A

Isothermal process:
A process during which the temperature T
remains constant.

Isobaric process:
A process during which the pressure P
remains constant.

Isometric : no V change

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17
Q

Diabatic vs adiabatic system

A

Dia -> E allowed in and out, (thermal contact w surroundings)

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18
Q

Endo vs exothermic process

A

Endo absorbs heat exo releases

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19
Q

Steady flow state

A

Steady fluid flow through a control volume
* Total volume, mass, and energy are constant
* Properties at any one point are constant
* Distribution of properties may be non-uniform

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20
Q

Abs, gauge and vacuum pressure

A

Absolute pressure:
The actual pressure at a given position. measured relative to absolute vacuum (i.e., absolute zero pressure).

Gauge pressure: The difference between the absolute pressure
and the local atmospheric pressure.

Vacuum pressures: Pressures below
atmospheric pressure.

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21
Q

Internal energy

A

Internal energy, U: The sum of all the microscopic forms of
energy-It comes from the total kinetic and potential energy of
molecules which composes the system (thermal, chem, nuclear, elec, magn)

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22
Q

2 thermal energies

A

Sensible energy: The portion of
the internal energy of a system
associated with the kinetic energies
of the molecules.

Latent energy: The internal energy
associated with the phase of a
system.

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23
Q

Chem E

A

Chemical energy: The internal
energy associated with the atomic
bonds in a molecule.

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24
Q

Nuclear Energy

A

Nuclear energy: The tremendous
amount of energy associated with
the strong bonds within the nucleus
of the atom itself.

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25
Q

What are the internal energy types

A

sensible, latent, chem, nu

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26
Q

Mechanical energy

A

Mechanical energy: The form of energy that can be converted to mechanical work completely and directly by an ideal mechanical device such as an ideal turbine.

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27
Q

Heat

A

Heat: energy transfer as a result of difference in temperature between system and surroundings.
- no phase change (from high to low temp)

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28
Q

Latent heat

A

The amount of energy absorbed or released during a phase-change process

latent heat of fusion: the amount of energy absorbed during melting is called the and is equivalent to the amount of energy released during freezing.

latent heat of vaporization is equivalent to the energy released during condensation

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29
Q

Work

A

Work: energy transfer due to other than a ΔT, W
-e.g. force over distance

30
Q

Conduction

A

Conduction: The transfer of energy from the more energetic
particles of a substance to the adjacent less energetic ones as a
result of interaction between particles (touching).

31
Q

Convection

A

Convection: The transfer of energy
between a solid surface and the
adjacent fluid that is in motion, and
it involves the combined effects of
conduction and fluid motion. The
faster the fluid motion, the greater
the heat transfer.

32
Q

Radiation

A

Radiation: The transfer of energy
due to the emission of
electromagnetic waves (or
photons).

33
Q

Electrical work

A

The generalized force is the
voltage (the electrical potential) and the
generalized displacement is the electrical charge.

34
Q

Magnetic work

A

The generalized force is the magnetic field strength
and the generalized displacement is the total magnetic dipole
moment.

35
Q

Electrical polarization work

A

The generalized force is the electric
field strength and the generalized displacement is the polarization of
the medium

36
Q

Mechanical forms of work

A

Shaft work, spring work, elastic work, stretching of liquid film, kinetic or potential work

37
Q

Zeroth law

A

For 3 systems, A, B and C, that are all adiabatically enclosed, if A is in thermal equilibrium with B which is also in equilibrium with C then A must be in thermal equilibrium with C

38
Q

First law of thermodynamics

A

energy can be neither created nor destroyed during a process; it can only change forms.

39
Q

Energy balance

A

The net change (increase or decrease) in the total energy of the system during a process
is equal to the difference between the total energy entering and the total energy leaving the system during that process

40
Q

Sign convention heat transfer work

A

Heat transfer to a system and work done on a system are positive; heat transfer from a system and work done by a system are negative.

41
Q

Pure substance

A

substance having a fixed chemical
composition throughout
* Single chemical element/compound
* Homogeneous mixture of various chemical elements or
compounds (air)
* A mixture of two or more phases of a pure substance

42
Q

Compressed/subcooled liquid

A

liquid not about to vaporize

43
Q

Saturated liquid

A

liquid about to vaporize

44
Q

Saturated liquid-vapour mixture

A

liquid and vapour phases coexist

45
Q

Saturated vapour

A

last drop of liquid just vaporized or vapour about to condense

46
Q

Superheated vapour

A

vapour not about to condense,
temperature of the vapour rises

47
Q

Saturation temperature

A

temperature at
which a pure substance
changes phase

48
Q

Saturation pressure

A

pressure at which a
pure substance changes
phase

49
Q

Specific heat

A

Energy required to raise the temperature of a unit mass of a substance by one degree.

50
Q

conservation of mass principle

A

Mass, like energy, is a conserved property, and it cannot be
created or destroyed during a process.

51
Q

Control volumes

A

Control volumes: Mass can cross the boundaries, and so we must keep track of the amount of mass entering and leaving the control volume.

52
Q

Steady flow process

A

the total amount of mass contained within a control volume
does not change with time (mCV = constant).

53
Q

Carnot principles

A
  1. The efficiency of an irreversible heat engine is always less than the efficiency of a reversible one operating between the same two reservoirs.
  2. The efficiencies of all reversible heat engines operating between the same two reservoirs are the same.
54
Q

Reversible vs irreversible processes

A

Reversible (Ideal) process
Can be completely reversed with no net
effect on its surroundings
* Final state = initial state for system, surroundings

Irreversible (real) process
* If the system and surroundings cannot be returned to their respective original states without leaving any trace on the surroundings
* Final state = initial state for system
* Final state ≠ initial state for surroundings

55
Q

Clausian statement (2nd law)

A

It is impossible to construct a device that operates in a cycle and produces no effect other than the transfer of heat from a lowertemperature body to a higher-temperature body.

56
Q

Kelvin-Planck statement (2nd law)

A

It is impossible for a cyclic
device to exchange heat with a
single reservoir and produce a
net amount of work.

57
Q

Second law

A

Heat always moves from hotter objects to colder objects,

58
Q

Major uses of second law

A
  1. may be used to identify the direction of processes.
  2. energy has quality as well as quantity.
  3. used in determining the theoretical limits for the performance of commonly used engineering systems, (heat engines and refrigerators)
59
Q

Reservoir

A

Body with large thermal energy capacity that can supply or absorb heat with no noticeable change in temperature

Source: Reservoir that supplies energy as heat
Sink: Reservoir that absorbs energy as heat

60
Q

Heat engine

A

device that converts heat to work.
* Receives heat from high-temperature source (solar energy, oil furnace, nuclear reactor, etc.)
* converts part of this heat to mechanical work (e.g. shaft work)
* Rejects the remaining waste heat to a low- temperature sink (the atmosphere, rivers, etc.).
* Operates on a cycle.

61
Q

Refrigerators

A

device that transfers heat from a low- temperature medium to a high-temperature

62
Q

Refrigerant

A

The working fluid that is used in the refrigeration cycle

63
Q

Irrerversibilities

A

Factors that cause process to be irreversible (friction, unrestrained expansion, mixing of two fluids, heat transfer across a finite temperature difference, electric resistance, inelastic deformation of solids, and chemical reactions)

64
Q

Types of reversibilities

A

Internally reversible process
(No irreversibilities occur within the system boundary during the process, Quasi-equilibrium process)

Externally reversible: No irreversibilities occur outside the system boundary. (Heat transfer across infinitely small temperature difference)

Totally reversible or simply reversible process: No irreversibilities within the system or its surroundings. (no heat transfer through a finite temperature difference, no nonquasi-equilibrium changes, and no friction or other dissipative effects)

65
Q

Ideal gas characteristics

A

gas particles = negligible volume in comparison with overall gas volume.

equally sized and do not have intermolecular forces (attraction or repulsion) with other gas particles.

move randomly in agreement with Newton’s Laws of Motion.

perfect elastic collisions with no energy loss.

66
Q

Carnot heat-engine

A

most efficient heat engine (totally reversible)

67
Q

Clausius inequality

A

The cyclic integral deltaQ/T is always less than or equal to zero (equal for totally reversible)

spontaneous systems heat flows from hot to cold

68
Q

Entropy characteristics

A

State property
(Dec if heat removed from syst. Inc if heat added)
Entropy change can be negative during process, butt entropy generation always + (due to irreversibilities)

69
Q

Pure substance

A

substance having a fiexd chemical composition throughout (sing element/mol, homogenous mixture of various ele/mol, 2 or more phases of pure sub)

70
Q

Flow work

A

Flow work, also known as “flow energy” or “displacement work”, is the work done by a fluid as it flows through a control volume, pushing a piston or turning a turbine. W=PV

71
Q

Boundary work

A

Boundary work, also known as “pressure-volume work” or “mechanical work”, is the work done by a system as it changes its volume while exerting a pressure against a boundary, such as a piston or a wall. int(PdV)

Physics (6 decks)

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